Synthesis, Complexation, and Coordination Oligomerization of 1,8

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Inorg. Chem. 2003, 42, 4346−4354

Synthesis, Complexation, and Coordination Oligomerization of 1,8-Pyrazine-Capped 5,12-Dioxocyclams Louis S. Hegedus,* Michael J. Sundermann, and Peter K. Dorhout Department of Chemistry, Colorado State UniVersity, Fort Collins, Colorado 80523 Received March 11, 2003

(Methyl)(methoxy)-5,12-dioxocyclam 1 was alkylated on the secondary amines (capped) with 2,6-bis(bromomethyl)pyrazine. The resulting macrocycle was complexed to copper(II) to produce a five-coordinate complex 5a which was fully characterized by a range of spectroscopic methods (IR, UV−vis, ESR) as well as by X-ray crystallography. The structure of this complex is similar to the previously reported pyridine complex, with the five-coordinate copper having distorted square pyramidal geometry and a Cu−Pz bond length of 2.125 Å. Attempts to prepare this same complex under microwave irradiation instead produced a trinuclear complex 6a having an octahedral copper(II) center complexed to two pyrazine−cyclam copper units through the amide carbonyl oxygen and the methoxyl group oxygen of the cyclam unit. The X-ray crystal structure of the trinuclear complex showed extensive distortion in the cyclam rings. The remote nitrogen of pyrazine−cyclam complex 5a was capable of coordinating an additional metal. Treatment with RuCl2(DMSO)4 or Rh2(OAc)4, respectively, produced trimetallic Cu−Ru−Cu complex 7 or tetrametallic Cu−Rh−Rh−Cu complex 8. The latter was fully characterized, including an X-ray crystal structure, and had two pyrazine−cyclam complexes bridged by a Rh2(OAc)4 unit through the remote pyrazine nitrogens. There was little distortion in the pyrazine−cyclam copper units as compared to complex 5a: the four metals were collinear, and the two cyclam units were eclipsed. All of the copper complexes were subjected to cyclic voltametry measurements, and no reversible redox changes were observed. Magnetic measurements of 6a and 8 showed the copper atoms to be weakly antiferromagnetically coupled.

Introduction Coordination polymers are multimetallic assemblies resulting either from the complexation of coordinating groups from a monomeric coordination complex to other metal centers, or, more commonly, by the reaction of polydentate ligands with metal complexes having multiple available coordination sites. The resulting arrays are connected by metal-ligand bonds rather than by the covalent bonds utilized in organic polymers. Over the past decade, coordination polymers have undergone development in a number of different directions. Major advances in the utilization of coordination polymerization for the self-assembly of supramolecular nanostructures have been made.1-3 Many have host-guest properties and can act as synthetic receptors4 or coordination complex analogues of zeolites.5 When the ligands bridging the metal * To whom correspondence should be addressed. E-mail: hegedus@ lamar.colostate.edu. (1) For recent reviews, see: (a) Leininger, S.; Olenyuk, B.; Stang, P. J. Chem. ReV. 2000, 100, 853. (b) Swiegers, G. F.; Malefetse, T. J. Chem. ReV. 2000, 100, 3483-3537. (c) Navarro, J. A. R.; Lippert, B. Coord. Chem. ReV. 2001, 222, 219.

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centers can transmit electronic information, the resulting coordination polymers may have unusual optical, magnetic, (2) For comprehensive monographs, see: (a) Transition Metals in Supramolecular Chemistry; Fabrizzi, L., Poggi, A., Eds.; Kluwer Academic Publisher: Dordrecht, The Netherlands, 1994. (b) Transition Metals in Supramolecular Chemistry; Sauvage, J. P., Ed., Wiley: Chichester, U.K., 1999. (c) ComprehensiVe Supramolecular Chemistry; Lehn, J. M., Chair, Ed.; Atwood, J. L., Davis, J. E. D., McNicol, D. D., Vogtl, F., Executive Eds.; Pergamon: Oxford, U.K., 1996; Vol. 1, p 1. (3) For reviews, see: (a) References 1a-c. (b) Fujita, M. Chem. Soc. ReV. 1998, 27, 417. (b) Stang, P. J.; Olenyuk, B. Acc. Chem. Res. 1997, 30, 502. (c) Fujita, M.; Ogura, K. Bull Chem. Soc. Jpn. 1996, 69, 1471. (4) Kitaura, R.; Fujimoto, K.; Noro, S.-i.; Kondo, M.; Kitagawa, S. Angew. Chem., Int. Ed. 2002, 41, 133. (5) (a) Creutz, C.; Taube, H. J. Am. Chem. Soc. 1973, 95, 1086. (b) Kaim, W.; Klein, A.; Glockle, M. Acc. Chem. Res. 2000, 33, 755. (c) Na¨ther, C.; Jess, I.; Greve, J. Polyhedron 2001, 20, 1017. (d) Weber, A.; Ertel, T. S.; Reinohl, U.; Feth, M.; Bertagnoli, H.; Leuze, M.; Hanack, M. Eur. J. Inorg. Chem. 2001, 679. (e) ComprehensiVe Supramolecular Chemistry; Sauvage, J. P., Hoseeini, M. W., Eds.; Pergamon: Oxford, U.K., 1996; Vol. 9. (f) Ferigo, M.; Bonhote, P.; Marty, W.; StoeckliEvans, H. J. Chem. Soc., Dalton Trans. 1994, 1549. (g) Ito, T.; Hamaguchi, T.; Nagino, H.; Yamaguchi, T.; Kido, H.; Zavarine, I. S.; Richmond, T.; Washington, J.; Kubiak, C. P. J. Am. Chem. Soc. 1999, 121, 4625.

10.1021/ic030090j CCC: $25.00

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1,8-Pyrazine-Capped 5,12-Dioxocyclams

or electronic properties, as well as the potential to recruit several metal centers to interact with a single substrate in a catalytic process. This class of bridging ligands includes pyrazines,5 triazines and tetrazines,6 cyano7 and isocyano8 groups, and polyacetylene-linked bi- and terpyridines.9 Dioxocyclams10 are 14-membered tetraazomacrocycles having two secondary amine nitrogens and two amide nitrogens as part of the macrocycle periphery. They are intermediate between cyclic polyamines and cyclic peptides in their metal-complexation properties and are more selective than their tetramine relatives, the cyclams.11 The secondary amines in dioxocyclams are reactive nucleophiles and can be alkylated or acylated by appropriate electrophiles.12 The use of bis-electrophiles results either in linking two macrocycles through the amine nitrogens, or capping one face of the macrocycle across the same positions.13 Recently, an efficient synthesis of dioxocyclams has been reported from these labs,14 along with capping studies with 2,6-bis(bromomethyl)pyridine.15 By using pyrazine in place of pyridine, capped cyclams capable of coordinating metals both inside the capped macrocycle and outside the cavity through the pyrazine 4-nitrogen should be accessible. Since pyrazine can act as an electron π-mediator (an electronic coupling element between metals16), this would permit the synthesis of coordination oligomers containing multiple communicating metal centers having potentially useful electronic, optical, or catalytic properties. Results of synthetic studies addressing this issue are given here. (6) (a) See ref 5d. (b) Pohmer. J.; Hanack. M.; Barcina, J. O. J. Mater. Chem. 1996, 6, 957. (7) Geiss, A.; Vahrenkamp, H. Inorg. Chem. 2000, 39, 4029 and references therein. (8) Hanack, M.; Kamenzen, S.; Kamenzen, G.; Subramanian, L. R. Synth. Met. 2000, 110, 93. (9) (a) Baxter, P. N. W. J. Org. Chem. 2000, 65, 1257. (b) Ziessel, R.; Hissler, M.; El-ghazoury, A.; Harriman, A. Coord. Chem. ReV. 1998, 178-180, 1251. (10) Dioxocyclams have been extensively developed by Kimura. For reviews, see: (a) Kimura, E. In Crown Ethers and Analogous Compounds; Hiraoka, M., Ed.; Studies in Organic Chemistry 45; Elsevier: New York, 1992; p 381. (b) Kimura, E. Pure Appl. Chem. 1989, 42, 823. (11) For reviews, see: (a) Lindoy, L. F. Chemistry of Macrocyclic Ligand Complexes; Cambridge University Press: London, 1989. (b) Izatt, R. M.; Pawlak, K.; Bradshaw, J. S.; Bruening, R. L. Chem. ReV. 1995, 95, 2529. (c) Martell, A. E.; Hancock, R. D. Metal Complexes in Aqueous Solutions; Plenum Press: New York, 1996. (12) (a) For a review, see: Denat, F.; Brandes, S.; Guilard, R. Synlett 2000, 561-574. (b) Kurosaki, H.; Bucher, C.; Espinosa, E.; Barbe, J.-M.; Guilard, R. Inorg. Chim Acta 2001, 322, 145. (c) Kurosaki, H.; Yoshida, H.; Fujimoto, A.; Goto, M.; Shionoya, M.; Kimura, E.; Espinosa, E.; Barbe, J.-M.; Guilard, R. J. Chem. Soc., Dalton Trans. 2001, 898-901. (13) (a) Lachkar, M.; Guilard, R.; Atmani, D.; DeCian, A.; Fischer, J.; Weiss, R. Inorg. Chem. 1998, 37, 1575. (b) Brandes, S.; Denat, F.; Lacour, S.; Rabiet, F.; Barbette, F.; Pullumbi, P.; Guilard, R. Eur. J. Org. Chem. 1998, 2349. (c) Brandes, S.; Lacour, S.; Denat, F.; Pullumbi, P.; Guilard, R. J. Chem. Soc., Perkin Trans. 1 1998, 639. (d) Denat, F.; Lacour, S.; Brandes, S.; Guilard, R. Tetrahedron Lett. 1997, 38, 4417. (14) (a) Puntener, K.; Hellman, M. D.; Kuester, E.; Hegedus, L. S. J. Org. Chem. 2000, 65, 8301. (b) Kuester, E.; Hegedus, L. S. Organometallics 1999, 18, 5318. (c) Hsiao, Y.; Hegedus, L. S. J. Org. Chem. 1997, 62, 3586. (d) Dumas, S.; Lastra, E.; Hegedus, L. S. J. Am. Chem. Soc. 1995, 117, 3368. (e) Hegedus, L. S.; Moser, W. H. J. Org. Chem. 1994, 59, 7779. (f) Betschart, C.; Hegedus, L. S. J. Am. Chem. Soc. 1992, 114, 5010. (15) Wynn, T.; Hegedus, L. S. J. Am. Chem. Soc. 2000, 122, 5034. (16) Fagalde, F.; Katz, N. E. Polyhedron 1995, 14, 1213.

Experimental Section Acetonitrile was distilled over calcium hydride. Methanol was dried over molecular sieves. Carbon tetrachloride was used as received. NMR spectra were recorded on a Varian JS-300. Infrared spectra were recorded on a Nicolet Magna-IR 760 spectrometer. UV-vis spectra were recorded on an Agilent G1103A spectrometer. EPR spectra were recorded on a Bruker EMX EPR spectrometer. The light used for photolysis reactions was from a 500 W quartzhalogen shop light lamp by Regent Lighting Corporation, model PQ72. The microwave used was a Sharp model R-2208W. Electrochemical measurements were conducted with an EG and G, Princeton Applied Research, model 75 universal programmer, model 179 digital coulometer, and model 173 potentiostat/galvanostat. The complex was dissolved in a 0.1 M solution of tetrabutylammonium hexafluorophosphate in acetonitrile. The working electrode was either glassy carbon or platinum. The counter electrode was a platinum wire. The reference electrode was a silver wire. Potentials were calculated versus SCE. Cyclic voltammograms were obtained at a scan rate of 100 mV/s. Data were plotted with the x-axis equal to 100 mV/cm. X-ray crystallographic studies were performed on a Bruker Smart CCD diffractometer, and the intensity of the data set was integrated using Bruker SAINT software. The structures were solved using Bruker SHELXTL version 5.03 software. For magnetic measurements, powdered samples (5-20 mg) were held within gelatin capsules and suspended by a Teflon rod in a Quantum Design MPMS SQUID magnetometer. Samples were cooled to liquid He temperature, and a field of 1.0 T was applied. Magnetization curves indicated that this was a reasonable field for these studies. Susceptibility data were collected at 0.5 K intervals from 2 to 10 K, 1 K intervals from 10 to 40 K, and 5 K intervals to 300 K. Data were corrected for the core diamagnetism of the elements in the ligands as well as crystalline solvent molecules. Synthesis of 2,6-Bis(bromomethyl)pyrazine (2). A suspension of 2,6-dimethylpyrazine (0.804 g, 7.43 mmol), N-bromosuccinimide (3.30 g, 18.6 mmol), and benzoyl peroxide (36 mg, 0.15 mmol) in 40 mL of carbon tetrachloride was stirred under irradiation from two 500 W lamps for 2 h. The solution turned orange, then back to clear, and black solid formed on the surface of the flask. The suspension was filtered through filter paper, and the solvent was removed by rotary evaporation. The residue was purified by chromatography on silica gel (25% ethyl acetate/hexanes) to give 0.342 g (17%) of 2,6-bis(bromomethyl)pyrazine as a clear oil. The liquid is very unstable in the pure form and is used immediately. It can be stored in solution at -20 °C without appreciable decomposition for at least several weeks. Rf ) 0.20. 1H NMR (300 MHz, CDCl3) δ: 8.64 (s, 2H), 4.55 (s, 4H). 13C NMR (300 MHz, CDCl3) δ: 151.9, 143.9, 30.1. Synthesis of Pyrazine-Capped Centrosymmetric Dioxocyclam (4a). A solution of 2,6-bis(bromomethyl)pyrazine (31 mg, 0.12 mmol), sodium carbonate (49 mg, 0.46 mmol), and centrosymmetric dioxocyclam 3a (43 mg, 0.12 mmol) in 3 mL of acetonitrile was stirred under argon at reflux for 4 days. The solution was filtered through Celite, and the solvent was removed by rotary evaporation. The residue was purified by chromatography on silica gel (9% methanol/chloroform), followed by recrystallization from methylene chloride/hexanes, to give 37 mg (71%) of pyrazine-capped centrosymmetric dioxocyclam 4a. 1H NMR (300 MHz, CDCl3) δ: 8.95 (s, 1H), 8.33 (d, J ) 3 Hz, 2H), 7.34 (s, 1H), 4.12 (m, 4H), 3.45 (s, 3H), 3.23 (d, J ) 14 Hz, 2H), 3.01 (m, 5H), 2.66 (d, J ) 15 Hz, 1H), 2.52 (s, 3H), 2.31 (d, J ) 14 Hz, 1H), 1.47 (s, 3H), 1.45 (s, 3H), 1.42 (s, 3H), 1.36 (s, 3H), 1.22 (s, 3H), 1.16 (s, 3H). 13C NMR (300 MHz, CDCl3) δ: 173.2, 172.6, 158.4, 153.5, 142.0, Inorganic Chemistry, Vol. 42, No. 14, 2003

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Hegedus et al. 140.6, 82.8, 79.8, 74.9, 72.6, 67.6, 67.1, 65.0, 62.9, 56.2, 54.9, 52.1, 50.5, 26.5, 25.8, 23.6, 19.4. IR (film) ν: 1660 cm-1 (CO). Anal. Calcd for C24H40N6O4: C, 60.48; H, 8.46; N, 17.30. Found: C, 60.60; H, 8.34; N, 17.55. Synthesis of Copper Complex 5a. A solution of cyclam 4a (36 mg, 0.08 mmol), copper(II) tetrafluoroborate hexahydrate (137 mg, 0.398 mmol), and potassium carbonate (55 mg, 0.39 mmol) in 5 mL of methanol was stirred at reflux for 1 day. The suspension was filtered through Celite, and the solvent was removed in vacuo by rotary evaporation. The residue was recrystallized from methylene chloride/hexane to give 29 mg (68% yield) of green solid. Mp 210-211 °C. IR (film) ν: 1587 cm-1 (CO). UV-vis (methanol) 407 ( ) 264), 684 ( ) 115) nm. Crystal structure solved. Synthesis of Pyrazine-Capped C2 Symmetric Dioxocyclam 4b. A solution of 2,6-bis(bromomethy)pyrazine (467 mg, 1.74 mmol), sodium carbonate (615 mg, 5.80 mmol), and C2 symmetric dioxocyclam 3b (540 mg, 1.45 mmol) in 25 mL of acetonitrile was stirred at reflux for 4 days. The solution was filtered through Celite, and the solvent was removed by rotary evaporation. The residue was purified by chromatography on silica gel (3% methanol/ chloroform) to give 42 mg (6%) of pyrazine-capped C2 symmetric dioxocyclam capped from the methoxy side (4c), 192 mg (28%) of pyrazine-capped C2 symmetric dioxocyclam capped from the methyl side (4b), and 258 mg of starting cyclam, making the total yield 65% based on recovered starting material. Data for major product (Me side) follow. 1H NMR (300 MHz, CDCl3) δ: 8.07 (s, 2H), 7.95 (s, 2H), 3.94 (dd, J ) 16.5, 40.0 Hz, 4H), 3.31 (s, 6H), 3.16 (d, J ) 15.0 Hz, 2H), 2.92 (d, J ) 14.7 Hz, 2H), 2.80 (d, J ) 13.8 Hz, 2H), 2.67 (d, J ) 13.5 Hz, 2H), 1.22 (s, 12H), 1.11 (s, 6H). 13C NMR (300 MHz, CDCl3) δ: 172.5, 149.9, 140.1, 83.3, 70.4, 66.6, 63.9, 54.0, 51.4, 29.0, 25.1, 20.2. IR (film) ν: 1653 cm-1 (CO). Anal. Calcd for C24H40N6O4: C, 60.48; H, 8.46; N, 17.63. Found: C, 60.13; H, 8.06; N, 17.30. Synthesis of Copper Complex 5b. A solution of 4b (28.0 mg, 0.059 mmol), copper(II) tetrafluoroborate hexahydrate (101 mg, 0.294 mmol), and potassium carbonate (40.6 mg, 0.294 mmol) in 10 mL of methanol was stirred at reflux for 2 days. The suspension was filtered through Celite, and the solvent was removed in vacuo by rotary evaporation. The residue was recrystallized with methylene chloride and filtered through a plug of alumina, leaving 22.0 mg (70% yield) of green solid. IR (film) ν: 1587 cm-1 (CO). UVvis (methanol) 756 ( ) 119) nm. HRMS (FAB+) Calcd for C24H38CuN6O4: 537.2251. Found: 537.2260. Synthesis of Tris-Copper Complex 6a. A solution of 4a (50.2 mg, 0.105 mmol), copper(II) tetrafluoroborate hexahydrate (182 mg, 0.526 mmol), and potassium carbonate (72.8 mg, 0.526 mmol) in 5 mL of methanol was placed in a Pyrex pressure tube. The solution was heated in a microwave (Sharp model R-220BW, power setting 1) for 60 s, and the solution turned bluish-purple. The suspension was filtered through Celite, and the solvent was concentrated in vacuo by rotary evaporation to 10 mL. The solution was allowed to stand for 3 days, and blue crystals grew from solution. The solid was collected on a filter and washed with methanol (3 × 10 mL). The solid was dried under high vacuum, to give 62.3 mg (86%) of blue crystals. Mp (decomp) 228 °C. IR (Nujol) ν: 1726, 1576 cm-1 (CO). UV-vis (methanol) 558 ( ) 637) nm. Crystal structure solved. Synthesis of Ruthenium-Bridged Copper Complex 7. A solution of copper complex 5a (25 mg, 0.046) and dichlorotetrakis(dimethyl sulfoxide)ruthenium(II) (11 mg, 0.023 mmol) in 11 mL of methanol was stirred for 16 h. The color of the solution turned from green to brown. Evaporation of the solvent gave a brown solid. IR (film): 1575 cm-1 (CO). UV-vis (methanol) 504 ( ) 668),

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632 ( ) 239) nm. MS (FAB+) Calcd for C52H88Cl2Cu2N12O10RuS2: 1404.5. Found: 1405.2 (max peak). Synthesis of Rhodium-Bridged Copper Complex 8. A solution of copper complex 5a (22 mg, 0.041 mmol) and rhodium(II) acetate (9 mg, 0.02 mmol) in 11 mL of methanol was stirred for 20 min. The color of the solution turned from green to brown. Evaporation of the solvent gave a brown solid. Recrystallization by slow evaporation of CH2Cl2/EtOAc gave dichroic green-brown crystals. IR (film): 1575 cm-1 (CO). UV-vis (methanol) 436 ( ) 739), 534 ( ) 340), 658 ( ) 222) nm. MS (FAB+) Calcd for C56H88Cu2N12O16Rh2: 1518.3. Found: 1518.7. Crystal structure solved.

Results and Discussion Synthesis and Complexation of Pyrazine-Capped Dioxocylam (4). Pyrazine-capped dioxocyclam 4 was synthesized following the procedure previously developed for the pyridine-capped analogue (eq 1).15 Although 2,6-bis(bromomethyl)pyridine is commercially available and quite stable, 2,6-bis(bromomethyl)pyrazine (2) must be synthesized. While pyrazine 2 is a literature compound,17 neither the details of its synthesis nor its characterization have been published. The most direct approach involves radical benzylic bromination. Treatment of 2,6-dimethylpyrazine with a slight excess of N-bromosuccinimide under incandescent light with benzoyl peroxide as the initiator produced the dibrominated pyrazine 2 in 17% isolated yield. As is typical for reactions of this type,5e reaction efficiency is compromised by overbromination. Further, 2 is relatively unstable to the reaction conditions and even decomposes when pure on standing. It is substantially more stable in solution and can be stored for weeks in solution at -20 °C. By limiting reaction times to 2-2.5 h, usable amounts of 2 are readily available. The only characterizable byproduct was the monobrominated compound which could be recycled. Treatment of centrosymmetric dioxocyclam 3a with 2 under standard15 capping conditions (acetonitrile, reflux 4 days, Na2CO3) produced pyrazine-capped dioxocyclam 4a in good yield. Since the tertiary amines cannot invert because of the rigid bridge, they are chiral, and a racemic mixture of 4a was obtained. Treatment with copper(II) tetrafluoroborate in methanol at reflux gave the desired pyrazine-capped dioxocyclam copper(II) complex 5a in good yield, as a bright green crystalline solid (eq 1). Recrystallization by slow evaporation from hexane/methylene chloride gave bright green crystals. The X-ray crystal structure and stereoview of 5a are shown in Figure 1, and selected bond lengths and angles are displayed in Table 1. The structural parameters resemble those of the closely related pyridine-capped copper dioxocyclam complex previously reported.15 The copper is clearly five-coordinate, with distorted square pyramidal (rather than trigonal bipyramidal) geometry (“equatorial” N-Cu-N angles of 154.8°, 107.9°, and 97.4° vs 180°, 90°, 90° for square pyramidal or 120°, 120°, 120° for trigonal bipyramidal). The pyrazine N5(17) Bridger, G. J.; Skerlj, R. T.; Padmanabhan, P.; Martellucci, S. A.; Henson, G. W.; Struyf, S.; Witurouw, M.; Schols, D.; DeClercq, E. J. Med. Chem. 1999, 42, 3971.

1,8-Pyrazine-Capped 5,12-Dioxocyclams Table 1. Selected Bond Lengths (Å) and Bond Angles (deg) for Complex 5a with Estimated Standard Deviations in Parentheses (amide) N(1)-Cu(1) (amine) N(2)-Cu(1) (amide) N(3)-Cu(1) (amine) N(4)-Cu(1) (Pz) N(5)-Cu(1) C(1)-O(1) C(6)-O(2) C(1)-N(1) C(6)-N(3)

1.936(11) 2.081(12) 1.975(11) 2.108(11) 2.125(12) 1.25(2) 1.227(18) 1.33(2) 1.343(18)

N(1)-Cu(1)-N(2) N(3)-Cu(1)-N(2) N(3)-Cu(1)-N(4) N(1)-Cu(1)-N(4) N(1)-Cu(1)-N(3) N(2)-Cu(1)-N(4) N(1)-Cu(1)-N(5) N(2)-Cu(1)-N(5) N(3)-Cu(1)-N(5) N(4)-Cu(1)-N(5)

97.9(5) 86.4(5) 99.4(5) 86.0(5) 154.8(5) 158.9(4) 97.4(5) 79.9(5) 107.9(5) 78.5(5)

of copper(II) tetrafluoroborate and sodium carbonate, in methanol in a pressure tube (eq 2). The resulting dark blue

Figure 1. ORTEP diagram and stereoview of 5a.

copper bond length of 2.125 Å is identical to that of the pyridine N5- copper bond length in the corresponding pyridine-capped complex,15 and similar to that found in pyrazine-bridged copper(II) complexes17 (2.0-2.1 Å).18

In an attempt to decrease the reaction time required for complexation, ligand 4a was irradiated for 2 min in a consumer microwave oven in the presence of a 5-fold excess

solution was filtered through a pad of Celite and allowed to stand for 2 days. Dark blue crystals of complex 6a were deposited, leaving a colorless solution. These crystals would not redissolve in methanol, even on extended heating, but readily dissolved to give a purple solution when a few drops of water or acetonitrile were added to the methanol suspension. The physical properties of this material suggested it might be an oligomer of 5a, formed by the coordination of the remote pyrazine N of one molecule to the copper of another. However, the X-ray crystal structure of 6a, displayed in Figure 2 with bond lengths and angles in Table 2, showed otherwise. The complex consists of two units of pyrazine-capped dioxocyclam copper complex 5a bridged by a third copper through one of the amide carbonyl groups and a methoxy group of the cyclam. The coordination sphere of the central copper is completed by two axial methanols. Since racemic 5a was used, diastereoisomers of 6a should be formed in equal amounts. The crystal structure is that of the centrosymmetric diastereoisomer.29 Complex 6a has a number of unusual features. It only forms under microwave irradiation. Prolonged heating (methanol at reflux 24 h) of the starting materials only produces (18) (a) Adachi, K.; Sugiyama, Y.; Kumagai, H.; Inoue, K.; Kitagawa, S.; Kawata, S. Polyhedron 2001, 20, 1411. (b) Darriet, J.; Haddad, M. S.; Duesler, E. N.; Hendrickson, D. N. Inorg. Chem. 1979, 18, 2679.

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Figure 2. ORTEP diagram and stereoview of 6a (BF4- counterions omitted for clarity), Table 2. Selected Bond Lengths (Å) and Bond Angles (deg) for Complex 6a with Estimated Standard Deviations in Parentheses (amine) N(1)-Cu(1) (amide) N(2)-Cu(1) (amine) N(3)-Cu(1) (amide) N(4)-Cu(1) (Pz) N(5)-Cu(1) (bound CO) C(8)-O(2) (free CO) C(17)-O(4) (bound CN) C(8)-N(2) (free CN) C(17)-N(4) (bound OMe) C(9)-O(3) (free OMe) C(2)-O(1) O(2)-Cu(2)

2.051(3) 1.925(3) 2.043(3) 2.309(3) 1.905(3) 1.279(4) 1.209(5) 1.300(4) 1.394(5) 1.470(4) 1.431(4) 1.895(2)

O(3)-Cu(2) O(5)-Cu(2) N(1)-Cu(1)-N(2) N(2)-Cu(1)-N(3) N(3)-Cu(1)-N(4) N(1)-Cu(1)-N(4) N(1)-Cu(1)-N(3) N(1)-Cu(1)-N(4) N(1)-Cu(1)-N(5) N(2)-Cu(1)-N(5) N(3)-Cu(1)-N(5) N(4)-Cu(1)-N(5)

2.040(2) 2.322(4) 90.20(11) 101.96(11) 82.30(11) 93.76(11) 167.28(11) 125.50(11) 85.07(12) 134.53(12) 83.72(12) 99.95(12)

complex 5a. Although pyrazine is an excellent ligand for copper(II) and many pyrazine-bridged copper(II) complexes are known,18,19 the third copper in complex 6a incorporates into the amide carbonyl/methoxy site rather than the available pyrazine site. Complex 6a has additional amide carbonyl/ methoxy sites on each cyclam ring, yet these did not complex additional copper to give oligomers despite the presence of excess copper tetrafluoroborate. Only one such site on each cyclam was coordinated. The bridging copper causes large distortions in the pyrazine-capped cyclam portion of the molecule, relative to complex 5a. As might be expected, complexation of one of the amide groups has a profound effect on the copper-amide nitrogen bond lengths, slightly shortening that to the coordinated amide (1.925 vs 1.936 Å in 5a) and dramatically lengthening that to the free amide to 2.309 Å: a 0.4 Å increase! The coordinated amide carbonyl CO bond is lengthened (1.279 Å vs 1.230 Å in 5a), and the free CO bond is shortened (1.209 Å). Similarly, the coordinated amide carbonyl C-N bond is shortened (1.300 Å vs 1.33 Å in 5a), and the free C-N bond is lengthened (1.394 Å). The pyrazine-copper bond length in 6a is shortened substantially (1.905 vs 2.125 Å in 5a), and the pyrazine ring is bent away (19) For recent examples, see: (a) Pickardt, J.; Staub, B. Z. Naturforsch., B.: Chem. Sci. 1997, 52, 1456-1460. (b) Dong, Y.-B.; Smith, M. D.; Layland, R. C.; zur Loye, H.-C. Inorg. Chem. 1999, 38, 5027. (c) Kwiatkowski, E.; Romanowski, G.; Nowicki, W.; Suwinska, K. Polyhedron 2001, 20, 1097.

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from the bridging amide nitrogen ([N(2)-Cu-N(5)] e 134.5° vs 107.9 Å in 5a). In addition, the cyclam ring is remarkably distorted from the relative planarity observed for complex 5a [(N(1)-Cu-N(3); N(2)-Cu-N(4) ≈ 160° for 5a vs 167° and 125° for 6a]. The geometry about the cyclam-copper is a distorted trigonal bipyramid, with equatorial bond angles of 125.5°, 134.5°, and 99.5° (vs 120° for trigonal bipyrimidial) and an “axial” bond angle of 167° versus 180° for trigonal bipyramidal. Finally, all three copper atoms are collinear, and the two pyrazine moieties are still available for further metal coordination, making 6a a potential building block for coordination oligomers. Related copper(II) trinuclear species have been reported for copper(II) complexes of 1,4,8,11-tetraazacyclotetradecane-2,3-dione20 and bis(3-aminopropyl)oxamide.21 In these cases, the bridging copper atom is coordinated to the two adjacent carbonyl groups of the oxamide. A less closely related tetracopper species involving linkage through a single coordinated amide carbonyl group of a 5,12-dioxocyclam has also recently been reported.22 For comparison purposes, the C2 symmetric cyclam 3b was also capped with pyrazine (eq 3). In this case, the two

faces of the cyclam are diastereotopic rather than enantiotopic, and the two possible diastereoisomers were obtained in 67% yield as a 1:4.5 mixture of diastereoisomers. Copper was introduced into the major (capping from the methyl face) diastereoisomer 4b as shown in eq 3, giving a bright green complex, 5b. Although copper(II) preferred amide coordination over pyrazine coordination in the formation of 6a, the free nitrogen in the pyrazine ring of complex 5a was capable of additional (20) Cronin, L.; Mount, A. R.; Parsons, S.; Robertson, N. J. Chem. Soc., Dalton Trans. 1999, 1925. (21) Journaux, Y.; Sletten, J.; Kahn, O. Inorg. Chem. 1986, 25, 439. (22) Goeta, A. E.; Howard, J. A. K.; Maffeo, D.; Puschmann, H.; Williams, J. A.; Gareth, Yufit, D. S. J. Chem. Soc., Dalton Trans. 2000, 1873. Trinuclear copper(II) complexes are also known for their distantly related bis-oximato ligands (Gao, E.-Q.; Zhao, Q.-H.; Tang, D.-Z.; Jiang, Z.-H.; Yan, S.-P. J. Chem. Soc., Dalton Trans. 2001, 1537) and dithiooxamido ligands (Veit, R.; Girerd, J.-J.; Kahn, O.; Robert, F.; Jeannin, Y. Inorg. Chem. 1986, 25, 4175).

1,8-Pyrazine-Capped 5,12-Dioxocyclams

coordination. Treatment of 5a with RuCl2(DMSO)4 or Rh2(OAc)4 produced tri- and tetrametallic complexes 7 and 8 with Ru or Rh bridging two units of complex 5a through the 4-position of pyrazine (eq 4). The Cu2Ru complex 7 was

characterized mainly by its mass spectrum, which had a parent peak cluster at m/z 1405 with the intensity pattern calculated for the assigned structure having two copper atoms and one ruthenium atom. Fragment clusters at m/z 1343 (pMe2S), m/z 1327 (p-DMSO), and m/z 539 (complex 5a) all were consistent with the assigned structure. The Cu2Rh2 complex 8 crystallized as dichroic brown-green crystals. The X-ray crystal structure of 8 is shown in Figure 3, with bond lengths and angles in Table 3. Again, since racemic 5a was used, diastereoisomers are expected. Again, the centrosymmetric diastereoisomer crystallized.29 In contrast to complex 6a, which displayed profound structural changes in the pyrazine-capped copper dioxocyclam unit relative to complex 5a, that same unit in complex 8 remained virtually unchanged. All bond lengths in the copper unit of 8 are within 0.04 Å of those in unbound 5a, and the biggest bond angle difference is 3°. Even the copper-pyrazine nitrogen bond length remained unchanged notwithstanding the fact that the pyrazine is now complexed to two metals. The pyrazine nitrogen-rhodium bond length (2.249 Å) is very close to that (2.231 Å) observed in the simple bis-pyridine adduct of Rh2(OAc)4,23 and the rhodiumrhodium bond lengths are very similar (2.389 Å for 8 vs 2.396 Å).24 Spectroscopic Studies. The spectroscopic parameters for compounds 4-8 are presented in Table 4; crystallographic details for 5-8 are available in Table 5. The most significant feature of the infrared spectra is the carbonyl stretching frequency for the amide group. For the (23) Koh, Y. B.; Christoph, G. G. Inorg. Chem. 1978, 17, 2590. For Rh(II) dimer bridged pyridyl porphyrins, see: Schaivo, S. L.; Serroni, S.; Puntoriero, F.; Tresoldi, G.; Piraino, P. Eur. J. Inorg. Chem. 2002, 79. For pyrazine-bridged rhodium(II) carboxylates, see: Mori, W.; Hoshino, H.; Nishimoto, Y.; Takamizawa, S. Chem. Lett. 1999, 331. (24) Rhodium(II) acetate also complexes isonitriles: Eagle, C. T.; Farrar, D. G.; Pfaff, C. U.; Davies, J. A.; Kluwe, C.; Miller, L. Organometallics 1998, 17, 4523. It also complexes nitriles: Miyasaka, H.; Campos-Fernandez, C. S.; Galan-Mascaros, J.; Dunbar, K. R. Inorg. Chem. 2000, 39, 5870.

Figure 3. ORTEP diagram and stereoview of complex 8. Table 3. Selected Bond Lengths (Å) and Bond Angles (deg) for Complex 8 with Estimated Standard Deviations in Parentheses N(1)-Cu(2) N(2)-Cu(2) N(3)-Cu(2) N(4)-Cu(2) N(5)-Cu(2) C(4)-O(2) C(12)-O(4) N(6)-Rh(I) Rh(I)-Rh(1A)

1.945(5) 2.112(4) 1.935(5) 2.103(4) 2.122(4) 1.243(6) 1.239(7) 2.249(4) 2.389(1)

N(1)-Cu(2)-N(2) N(3)-Cu(2)-N(2) N(3)-Cu(2)-N(4) N(1)-Cu(2)-N(4) N(3)-Cu(2)-N(1) N(4)-Cy(2)-N(2) N(1)-Cu(2)-N(5) N(2)-Cu(2)-N(5) N(3)-Cu(2)-N(5) N(4)-Cu(2)-N(5) N(6)-Rh(I)-Rh(1A)

85.70(18) 99.21(18) 84.75(18) 99.85(18) 155.92(19) 157.23(17) 104.81(18) 78.52(16) 99.27(18) 78.71(16) 178.31(12)

uncomplexed ligands, this falls in the range 1653-1667 cm-1 and includes the uncapped cyclams 3a,3b, the pyrazinecapped cyclams 4a,4b, and the corresponding pyridinecapped centrosymmetric ligand analogue of 4a.15 Introduction of copper(II) into these ligands shifts this absorption to the range 1575-1590 cm-1. Further complexation of the exocyclic nitrogen of the pyrazine (complexes 6-8) causes only a minor shift, from 1590 to 1575 cm-1. As might be expected, the most profound changes were observed for complex 6a, in which one of the amide carbonyl groups is coordinated through oxygen to another copper. In this instance, two carbonyl absorptions were observed, at 1725 and 1575 cm-1. Little information concerning the relative donor-acceptor capabilities of the various capping species Inorganic Chemistry, Vol. 42, No. 14, 2003

4351

Hegedus et al. Table 4. Spectroscopic Properties for Compounds 3-8 ESRa compd

IR, νcm-1

3a 3b 3a-Cu(II) 3b-Cu(II) 4a 4b 5a

1664 1667 1575 1583 1660 1653 1590

5b

1586

6a 7

1725 1575 1575

8

1575

a

λmax, nm ()b

giso

Aiso

G, cm-1

522(75) 631(183)

2.1241 2.1139

97 100

(9.47 × 10-3) (9.76 × 10-3)

407(sh) 684(116) 400(s) 756(119) 407(sh) 558(637) 504(668) 632(239) 436(739) 534(340) 658(222)

2.1368

103

(1.00 × 10-2)

2.1553

82

(8.00 × 10-3)

2.1360

90

(8.78 × 10-3)

2.1347

100

(9.76 × 10-3)

Spectra run in 3:1 CH2Cl2/PhH. b Spectra run in methanol.

Table 5. Crystallographic Data 5 empirical formula fw T (K) wavelength (Å) cryst syst space group unit cell dimensions a (Å) b (Å) c (Å) R (deg) β (deg) γ (deg) V (Å3), Z dcalcd (Mg/m3) abs coeff (mm-1) GOF of F2 final R indicesa [I > 2σ(I)] R indices (all data)

6

8

C24H38CuN6O4 538.14 298(2) 0.71073 triclinic P1h

C32H50CuN6O10Rh 845.23 183(2) 0.71073 triclinic P1h

C25H41B2Cu1.5F8N6O5 742.80 298(2) 0.71073 monoclinic P21/c

9.2796(6) 15.0482(10) 18.7680(11) 89.117(2) 90.000(2) 72.0410(10) 2492.8(3), 4 1.434 0.919 1.112 R1 ) 0.1025, wR2 ) 0.1866 R1 ) 0.1831, wR2 ) 0.2317

9.533(3) 14.048(5) 14.153(5) 96.406(6) 93.866(6) 104.369(6) 1815.7(10), 2 1.546 1.103 0.967 R1 ) 0.0467, wR2 ) 0.1132 R1 ) 0.0744, wR2 ) 0.1238

11.2129(16) 13.640(2) 21.933(3) 90 97.366(3) 90 3326.8(8), 4 1.483 0.745 1.042 R1 ) 0.0426, wR2 ) 0.1106 R1 ) 0.0561, wR2 ) 0.1171

a R ) ∑|F | - |F ||/∑|F |. R ) [∑[w(F - F 2)2]/∑[w(F 2)2]]1/2; w ) o c o w o c o 4Fo2/σ2(Fo2).

can be inferred from the infrared data because of the substantial changes in geometry about copper caused by a rigid bridge between the two amine nitrogens. The visible spectra also showed responses to changes in geometry about copper. The copper complex of centrosymmetric ligand 3a was pale violet and had a broad, weak ( ) 75) absorption around 522 nm. In contrast, the copper complex of C2 symmetric ligand 3b was dark purple and had a more intense ( ) 183) absorption at 631 nm. The bright green pyrazine-capped complexes 5a and 5b had pronounced shoulders at 407 and 400 nm, respectively, and moderate absorptions at 684 nm ( ) 116) and 756 nm ( ) 119), respectively. This large red shift may be, in part, due to alkylation of the amine nitrogens, weakening in-plane bonding to copper,25 but a substantial portion of it must be due to the presence of the cap. For comparison, the green pyridine-capped version of 5a15 has an absorption at 678 nm ( ) 72). The bright blue tris-copper complex 6a had a shoulder at 407 nm and a fairly strong absorption at 558 nm

4352 Inorganic Chemistry, Vol. 42, No. 14, 2003

( ) 637). Although UV spectra were not reported for the related20,21 2,3-dione tris-copper complexes already discussed, they are likely to have quite different visible spectra since they are reported to be deep red in both the crystalline state and in solution. The ruthenium-bridged complex 7 had an intense absorption at 504 nm ( ) 668) (vs 495 nm [( ) 573) for Ru(dmso)4Cl2]) and a weaker one at 632 nm ( ) 239), indicating that both partners were affected by additional coordination. The dirhodium bridged complex 8 had three absorptions, at 436 nm ( ) 739), 534 nm ( ) 340), and 658 nm ( ) 222) vs 364 nm (sh) and 546 nm for Rh2(OAc)4. The isotropic ESR spectra of the above copper complexes are also informative.26 The uncapped copper complexes of 3a and 3b had very similar ESR spectra, typical27 for square planar copper(II) complexes, with four equally spaced absorptions due to the interaction with the copper(II) nucleus (J ) 3/2). Hyperfine structure was seen on the high field peaks, but not the low field peaks. The ESR spectrum of C2 symmetric pyrazine capped complex 5b similarly had four equally spaced absorptions but lacked any hyperfine structure. In sharp contrast, centrosymmetric analogue 5a had a single broad absorption (giso ) 2.1368, Aiso ) 103) with a slight shoulder downfield from the main peak, and no features upfield. This is virtually identical to the centrosymmetric pyridine-capped complex (giso ) 2.1367). Both of these complexes have ESR spectra that stand in contrast to those observed for copper(II) complexes of 5,7-dioxocyclams having a quinoline25a (four peaks, giso ) 2.094) or a pyridine25b (four peaks, giso ) 2.096) pendant from one of the cyclam ring amine nitrogens. Complexation of the pyrazine to ruthenium(II) (complex 7) or rhodium(II) (complex 8) caused very little change in the ESR spectrum of 5a. The ESR spectrum of complex 7 is similarly broad (giso ) 2.1360) with slight shoulders both up and downfield of the main absorption, while that of complex 8 (giso ) 2.1347) had a weak downfield absorption in place of the downfield shoulder of complex 5a. Electrochemical Studies. The electrochemistry of copper(II)-cyclam and -oxocyclam complexes has been studied extensively by Kimura et al.28 Although the parent cyclamcopper(II) complex undergoes irreversible oxidation, systematic replacement of amine groups by amide groups results in increasing net stabilization of the +3 oxidation state of copper. As a consequence, the monooxocyclam-copper(II) complex has a quasireversible oxidation wave at +0.86 V (25) (a) Bu, X.-H.; An, D. L.; Chen, Y. T.; Shinoyo, M.; Kimura, E. J. Inclusion Phenom. 1997, 27, 245. This paper reports a red shift from 516 to 576 nm for related pendant quinoline-copper dioxocyclam complexes. See also: (b) Bu, X.-H.; An, D. L.; Cao, X.-C.; Zhang, R. H.; Clifford, T.; Kimura, E. J. Chem. Soc., Dalton Trans. 1998, 2247. (c) Bu, X.-H.; Cao, X.-C.; An, D. L.; Zhang, R. H.; Thomas, C.; Kimura, E. J. Chem. Soc., Dalton Trans. 1998, 433. (26) Full ESR spectra are contained in the Supporting Information associated with this paper. (27) Drago, R. S. Physical Methods for Chemists, 2nd ed.; Surfside: Gainesville, FL, 1992; p 590. From: Hasty, E. F.; Colburn, T. J.; Hendrickson, D. N. Inorg. Chem. 1973, 12, 2414. (28) Kimura, E.; Koike, T.; Machida, R.; Nagai, R.; Kodama, M. Inorg. Chem. 1984, 23, 4181. (29) For a detailed discussion of stereoisomerism in capped bis-cyclams, see ref 15.

1,8-Pyrazine-Capped 5,12-Dioxocyclams

(vs SCE), while the 1,3-dioxocyclam copper complex oxidizes at +0.64 V and the 1,3,7-trioxocyclam oxidizes at +0.43 V. Both the increased donor ability of deprotonated amides over amines, and the preference of square planar geometry of copper(III) species, accounts for this dramatic decrease in oxidation potential. Appending a 2-pyridylmethyl25b or an 8-quinolylmethyl25a group to an amine nitrogen of the 1,3-dioxocyclam copper(II) complex produced five-coordinate distorted square pyramidal complexes. This resulted in an increase in the oxidation potential to +0.83 V (vs SCE) and +0.78 V, respectively. The coordination of the pendant heterocycle stabilizes the +2 oxidation state. However, copper(III) tends to adopt square planar coordination in preference to fivecoordination, resulting in decoordination of the apical heterocycle upon oxidation and increasing the oxidation potential. The copper(II) complexes reported herein showed substantially different electrochemical behavior. The complex of uncapped C2 symmetric ligand 3b had a reversible oxidation wave at +0.49 V (vs SCE) similar to that observed for the 1,3-dioxocyclam already discussed.28 Surprisingly, the complex of the uncapped centrosymmetric ligand 3a underwent irreversible oxidation. Similarly, the pyridinecapped copper(II) complexes of 3a and 3b, the pyrazinecapped copper(II) complexes of the same ligands, and polymetallic complexes 5, 7, and 8, all underwent irreversible oxidation. This is consonant with the increase in oxidation potential caused by pendant ligands already discussed.25a,b The difference here is that, because of the rigid two-point attachment of the capping ligand, decomplexation to form a stabilized square planar copper(III) complex is not possible, and this oxidation state becomes inaccessible. Tricopper complex 6a showed an irreversible reduction peak at -0.99 V (vs Ag/AgO) with an associated oxidation peak at -0.58 V. This is very similar to that observed with the literature tricopper species already cited,20 which was attributed to reduction of only the central copper ion, with deposition on the electrode in a two electron process, followed by reoxidation to generate a copper(I) species. Neither oxidation nor reduction of the cyclam-bound copper was observed. Magnetic Properties. Magnetic Behavior of 6a. The copper(II) cyclam complex, 6a, resembles the cyclam complexes of Kahn21 and Robertson20 and the trinuclear Cu(II) complexes of Gao;22 however, 6a is unable to form a strong dimeric complex across the central copper atoms due to the methanol ligands coordinated in the solid state. Consequently, there is no Cu(2)-Cu(2) intermolecular separation near 3.2 Å as in their complexes. It was therefore anticipated that little or no intermolecular antiferromagnetic (AF) communication would be observed. However, the data at low temperatures do suggest that there is still a weak anitferromagnetic coupling between molecules in the crystal (J′ < 10 cm-1). The plot of susceptibility, χ, versus T, showed typical Curie-Weiss paramagnetic behavior with a room-temperature moment, µeff ) 3.07 µB, and a Weiss constant, θ ) -1.4, indicating a weak AF communication among centers. (A plot

Figure 4. Plot of χT versus T for complex 6a.

Figure 5. Plot of χT versus T for complex 8.

of χT versus T is shown in Figure 4.) This value is reasonable compared to a classical three-center S ) 1/2, µeff ) 2.996 µB. The plot shows that the moment decreases with temperature until about 100 K where the moment levels to 2.10 µB. This value is a bit high compared with a S ) 1/2 AF coupled system where µeff ) 1.73 µB. Nevertheless, the data are consistent with what others have observed for similar Cu(II) systems.20-22 At very low temperatures, an abrupt downturn in the χT data was observed, suggesting that there is a lower-lying AF state that is likely due to intermolecular interactions. This hypothesis is based on Kahn’s model for a weakly AF system with a low-lying coupling between two trinuclear copper complexes. Kahn’s coupling constant was J ) -2.9 cm-1; therefore, we conclude that the intermolecular coupling constant in our system is equally small. However, we have not been able to adequately model our data using the equations reported earlier21 to model J′, the intermolecular coupling constant. Magnetic Studies of 8. The magnetic susceptibility of 8 is displayed in Figure 5 as χT versus T. The sample showed classic Curie-Weiss behavior at low temperatures, with a very weak AF Weiss constant, θ ) -40 K. The χT plot illustrates a moment of µeff ) 2.41 µB at room temperature. This value is very close to the expected value for two S ) 1/ systems with one unpaired electron on each site and is 2 consistent with the picture of two Cu(II) d9 atoms not coupled through the Rh-Rh dimer, where the theoretical moment should be µeff ) 2.440 µB. This suggests that the localized, paired δ* electrons are not involved in any superexchange Inorganic Chemistry, Vol. 42, No. 14, 2003

4353

Hegedus et al. process at room temperature, unlikely in any event as the symmetry of the HOMO is not consistent with superexchange.30 At temperatures below 100 K, a downturn in the moment, nearly reaching zero at 25 K, was observed, suggesting that there is some coupling between the copper atoms either through the rhodium dimer or through space with other molecules in the unit cell. We are currently engaged in low-temperature ac susceptibility measurements to determine the nature of the low-temperature behavior in 8 and an attempt to model this magnetic data in an effort to evaluate the level of Cu-Cu coupling through the rhodium dimer.

nate to other metals, allowing 5a to be utilized as a subunit in coordination oligomers. This was demonstrated by the synthesis of tri- and tetrametallic complexes 7 and 8. Current studies are centering on the synthesis of bis-pyrizine-biscyclam ligands and complexes for the ultimate synthesis of more extended coordination oligomers.

Summary

Acknowledgment. Support for this research under Grant CHE-9908661 from the National Science Foundation is gratefully acknowledged. Mass spectra were obtained on instruments supported by National Institutes of Health shared instrumentation Grant GM 49631. Professor David Shultz, North Carolina State University, is acknowledged for his assistance in interpreting the magnetic measurements.

In summary, a pyrazine-capped 5,12-dioxocyclam was synthesized. Complexation to copper produced the expected mononuclear copper complex 5a under thermal conditions but the unusual tricopper species 6a under microwave irradiation. The remote pyrazine nitrogen of 5a can coordi-

Supporting Information Available: ESR spectra for complexes 3a, 3b, 5a, 5b, 7, and 8, and tables of crystal data, structure solutions and refinement, atomic coordinates, bond lengths and angles, and anisotropic thermal parameters for 5a, 6a, and 8. This material is available free of charge via the Internet at http://pubs.acs.org.

(30) Norman, J. G., Jr.; Kolari, H. J. J. Am. Chem. Soc. 1978, 100, 791.

IC030090J

4354 Inorganic Chemistry, Vol. 42, No. 14, 2003